A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 °C, and the following equilibrium is achieved: N2O4(g) ⇋ 2NO2(g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. 1.What is the equilibrium partial pressure of N2O4? 2.Calculate the value of Kp for the reaction.
A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 °C, and the following equilibrium is achieved: N2O4(g) ⇋ 2NO2(g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. 1.What is the equilibrium partial pressure of N2O4? 2.Calculate the value of Kp for the reaction.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 °C, and the following equilibrium is achieved: N2O4(g) ⇋ 2NO2(g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.
1.What is the equilibrium partial pressure of N2O4?
2.Calculate the value of Kp for the reaction.
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